Printed with permission of The Institute of Pure and Applied Physics (IPAP)

JAPANESE JOURNAL OF APPLIED PHYSICS
Vol.44, No.12 (2005) pp.8269-8285[Part1]

Invited Review Paper

TiO2 Photocatalysis:
A Historical Overview and Future Prospects
Kazuhito Hashimoto1,2, Hiroshi Irie2 and Akira Fujishima3

Photocatalysis has recently become acommon word and various products using
photocatalytic functions have been commercialized. Among many candidates for photocatalysts, TiO 2 is almost the only material
suitable for industrial use at present and also
probably in the future. This is because TiO2 has
the most efficient photoactivity, the highest
stability and the lowest cost. More significantly, it has been used as a white pigmentfrom ancient times, and thus, its safety tohumans and the environment is guaranteedby history. There are two types of photochemical reaction proceeding on a TiO 2
surface when irradiated with ultraviolet light.
One includes the photo-induced redox reactions of adsorbed substances, and the other isthe photo-induced hydrophilic conversion of
TiO2 itself. The former type has been known
since the early part of the 20th century, but
the latter was found only at the end of the
century. The combination of these two functions has opened up various novel applicationsof TiO2, particularly in the field of building
materials. Here, we review the progress of thescientific research on TiO2 photocatalysis as
well as its industrial applications, and describe
future prospects of this field mainly based on
the present authors’ work.
KEYWORDS:titanium dioxide, Honda–
Fujishima effect, photoelectrolysis, redox reaction, hydrophilic
conversion, environmental
application

1. Historical Background before Honda–Fujishima Effect
TiO2 powders have been commonly used
as white pigments from ancient times. They
are inexpensive, chemically stable and harmless, and have no absorption in the visible
region. Therefore, they have a white color.
However, the chemical stability of TiO2 holds
only in the dark. Instead, it is active under UVlight irradiation, inducing some chemical reactions. Such activity under sunlight was known
from the flaking of paints and the degradation of fabrics incorporating TiO2.1) Scientificstudies on such photoactivity of TiO2 havebeen reported since the early part of the 20th
century. For example, there was a report on
the photobleaching of dyes by TiO2 both invacuo and in oxygen in 1938.2) It was reported
that UV absorption produces active oxygen
species on the TiO 2 surface, causing thephotobleaching of dyes. It was also known
that TiO2 itself does not change through thephotoreaction, although the ``photocatalyst’’
terminology was not used for TiO 2 in thereport, but called a photosensitizer.
It is equivocal when and who started
utilizing first such a photochemical powerof TiO2 to induce chemical reactions actively,
but at least in Japan, there were a series ofreports by Mashio et al., from 1956, entitled``Autooxidation by TiO2 as a photocatalyst’’.3)
They dispersed TiO 2 powders into variousorganic solvents such as alcohols and hydrocarbons followed by the UV irradiation withan Hg lamp. They observed the autooxidation of solvents and the simultaneous formation of H 2O 2 under ambient conditions. It
is interesting to note that they had alreadycompared the photocatalytic activities ofvarious TiO2 powders using twelve types ofcommercial anatase and three types of rutile,and concluded that the anatase activity of
the autooxidation is much higher than that ofrutile, suggesting a fairly high degree of progress of the research.4) In those days, however,the photocatalytic power of TiO2 might haveattracted only partially limited scientists’ attention in the field of either catalysis or photochemistry, and the study of TiO2 photocatalysis
had not developed widely in either academic
or industrial society.

2. Water Photolysis with TiO2
Electrode in 1970s
In the late 1960s, one of the present
authors (AF) began to investigate the photoelectrolysis of water, using a single crystal
n-type TiO2 (rutile) semiconductor electrode,because it has a sufficiently positive valenceband edge to oxidize water to oxygen. It isalso an extremely stable material even in thepresence of aqueous electrolyte solutions,much more so than other types of semiconductor that have been tried. The possibility ofsolar photoelectrolysis was demonstrated forthe first time in 1969 with the system shownin Fig. 1, which was exposed to near-UV
light, and was connected to a platinum black
counter electrode through an electrical load.5)
Then, this electrochemical photolysis of water
was reported in Nature by analogy with anatural photosynthesis in 1972. 6) In thosedays, crude oil prices ballooned suddenly,
and the future lack of crude oil was a serious
concern. Thus, this became known as the timeof ``oil crisis’’. Therefore, this report attracted
the attention not only of electrochemists but

1 Research Center for Advanced Science and Technology, The University of Tokyo, 4-6-1 Komaba, Meguro-ku, Tokyo 153-8904, Japan
2 Department of Applied Chemistry, The University of Tokyo, 7-3-1 Hongo, Bunkyo-ku, Tokyo 113-8656, Japan
3 Kanagawa Academy of Science and Technology, 3-2-1 Sakado, Takatsu-ku, Kawasaki, Kanagawa 213-0012, Japan(Received August 11, 2005; accepted September 26, 2005; published December 8, 2005)©2005 The Japan Society of Applied Physics

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JSAP International No.14 (July 2006)

When the surface of the rutile TiO2 electrode was irradiated with light consisting of
wavelengths shorter than its band gap, about
415nm (3.0eV), photocurrent flowed from theplatinum counter electrode to the TiO2 electrode through the external circuit. The direction of the current revealed that the oxidation
reaction (oxygen evolution) occurs at the TiO2electrode and the reduction reaction (hydrogen
evolution) at the Pt electrode. This observation shows that water can be decomposed,using UV light, into oxygen and hydrogen,without the application of an external voltage,according to the following scheme.
TiO2 + hν → e– + h+
(at the TiO2 electrode)
2H2O + 4h+ → O2 + 4H+(at the Pt electrode)
2H+ + 2e– → H2

(1)
(2)
(3)

The overall reaction is
2H2O + 4hν → O2 + 2H2(4)

When a semiconductor electrode is in contact
with an electrolyte solution, thermodynamic
equilibration occurs at the interface. This may
result in the formation of a space-charge layer
within a thin surface region of the semiconductor, in which the electronic energy bands
are generally bent upwards and downwards
in the cases of the n- and p-type semiconductors, respectively. The thickness of thespace-charge layer is usually of the order of

1–103nm, depending on the carrier densityand dielectric constant of the semiconductor.
If this electrode receives photons with energies greater than that of the material bandgap, E G, electron–hole pairs are generated
and separated in the space-charge layer. In
the case of an n-type semiconductor, theelectric field existing across the space-charge
layer drives photogenerated holes toward theinterfacial region (i.e., solid–liquid) and electrons toward the interior of the electrode andfrom there to the electrical connection to theexternal circuit. The reverse process occurs
at a p-type semiconductor electrode. Thesefundamental processes of semiconductor
photoelectrochemistry have been discussed inmany recent reviews.7–11)

It is desirable that the band gap of thesemiconductor is near that for the optimum
utilization of solar energy, which would be
about 1.35eV. When semiconductor electrodes
are used as either photoanodes or photocathodes for water electrolysis, the bandgap
should be at least 1.23eV (i.e., the equilibrium
cell potential for water electrolysis at 25°C and1atm), particularly considering the existence ofpolarization losses due to, for example, oxygen
evolution. Although various semiconductors
with smaller band gaps were investigated,none succeeded for the water photoelectrolysis with visible light. This is because they werein most cases corroded in an aqueous electrolyte under irradiation, i.e., the photogenerated
holes oxidized the semiconductor itself.

If the conduction band energy E CB ishigher (i.e., closer to the vacuum level, or
more negative on the electrochemical scale)than the hydrogen evolution potential, photogenerated electrons can flow to the counterelectrode and reduce protons, resulting inhydrogen gas evolution without an applied
potential, although, as shown in Fig. 2, E CB
should be at least as negative as –0.4V versus
the standard hydrogen electrode (SHE) inacid solution or –1.2V (SHE) in alkaline solution. Among the oxide semiconductors, TiO2
(acid), SrTiO3, CaTiO3, KTaO3, Ta2O5, and ZrO2
satisfy this requirement. On the other hand,the employment of an external bias or of adifference in pH between the anolyte and thecatholyte is required in the case of other materials in order to achieve hydrogen evolution.

One of the other approaches to utilize
longer wavelength light could involve the dye
sensitization of TiO2. This approach, although
it is theoretically possible to use it for waterphotoelectrolysis, has practical problems, principally that most photosensitizer dyes would
be far too unstable under these conditions.
Therefore, the so-called regenerative photoelectrochemical cells, in which a single redox
couple exists, the reduced form is oxidized at
the TiO2 photoanode and the oxidized form isreduced at the counter electrode, were studied
intensively. Chlorophyll and various organicdyes, such as xanthene dyes, were used assensitizers, but neither the solar conversion
efficiency nor the stability of the dyes wasvery high in those days. It is, however, to beemphasized that this approach was intensively
researched later by Gratzel et al. using porous

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Fig.1. Schematic diagram of electrochemical photocell. (1) n-type
TiO2 electrode; (2) platinum black counter electrode; (3) ionicallyconducting separator; (4) gas buret; (5) load resistance; and (6) voltmeter.

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also of many scientists in a broad area, andnumerous related studies were reported in the
1970s.

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Fig.2. Schematic representation of photoelectrochemical water electrolysis using illuminated oxide semiconductor
electrode. An open circuit (or small current), pH 2, and illuminated conditions are shown for oxides with an ECB of-0.65V (SHE) and an EVB of 2.35V (SHE). With the open circuit, a small excess potential (0.15V) is available for H2 evolution, assuming a reversible counter electrode.

JSAP International No.14 (July 2006)

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TiO2 electrodes and ruthenium complexes assensitizers, and that the conversion efficiency
reached 10–11% in the 1990s.12,13)

3. Powdered TiO2 Photocatalysis in 1980s
The problem of light-assisted water splitting has also been focused in the late 1970s
with the photocatalytic approach, i.e., essentially with photoelectrochemistry but without
an external circuit. Conceptually, this is similar
to the process of corrosion, as being the
combination of two short-circuited electrochemical reactions. In the case of corrosion,
the two reactions might be anodic metal
dissolution together with either cathodic H2evolution or O 2 reduction. Photocatalytic
water splitting has been studied intensively
with powdered anatase TiO2 suspensions, with
Pt deposited on TiO2 as a cathodic catalyst.
Although there were several experiments forthe simultaneous production of H2 and O2 in
the powder systems, either such experiments
could not be reproduced or the reaction efficiency was very low.14)
Kawai and Sakata examined, in 1980,
the reasons why the water photolysis could
not proceed in the powder system, although
it could in the electrode one. They concluded
that the produced H2 and O 2 gases mightrecombine to regenerate water molecules
through the back reaction in the powder
system, because the production sites of eachgas are located close to each other. To solve
this problem, they added organic compounds
to the aqueous suspension of platinized TiO2.
In this case, water is reduced, producing H2
at the Pt sites and the organic compounds
are oxidized instead of water by photogenerated holes at the TiO2 sites. The H2 production proceeds surprisingly efficiently, with aquantum yield of more than 50% in the presence of ethanol.15) Most organic compounds,
including biomass-derived compounds andeven waste organisms, can enhance thehydrogen production efficiency. This is because
the redox potential for photogenerated holes
is +2.53V versus SHE, as shown in the energy
band diagram for TiO 2 (Fig. 3), and mostorganic compounds can be oxidized finally
into CO 2. In general, anatase ( E G = 3.2eV)
gives better results than rutile (EG = 3.0eV) forhydrogen production in powder photocatalysis. One of the main reasons for the higher

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JSAP International No.14 (July 2006)

efficiency is probably the higher reduction
potential of photogenerated electrons in theformer than in the latter, i.e., the bottom of
the conduction band of anatase is located 0.1V
more negative than that of rutile.16)
The first report on the efficient hydrogenproduction from water and organic compounds
was published in Nature at the time of thesecond oil crisis, and TiO2 photocatalysis drew
the attention of many people as one of thepromising methods for hydrogen production.
However, even though the reaction efficiency
is very high, TiO2 can absorb only the UV light
contained in a solar spectrum, which is only
about 3%. Therefore, from the viewpoint of H2
production technology, TiO2 photocatalysis is
not very attractive. Various other semiconductors with a small band gap, such as CdS and
CdSe, were investigated, but their efficiency
and stability were much lower than those of
TiO2, and the enthusiasm in the research of theH2 production was over in the middle of the
1980s.
Instead, the research shifted to the utilization of the strong photoproduced oxidation
power of TiO2 for the destruction of pollutants. The first such reports were those of Frankand Bard in 1977, in which they describedthe decomposition of cyanide in the presenceof aqueous TiO2 suspensions.17) In the 1980s,
detoxications of various harmful compounds
in both water and air were demonstratedusing powdered TiO 2 actively as potential
purification methods of waste water andpolluted air.18) When the purpose shifted tothe oxidation reaction of harmful compounds,�����������

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Fig.3.

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Schematic diagram of energy band for TiO2.

the reduction reaction was not necessarilyhydrogen production anymore. The platinization of TiO2 was not necessary in this case,and TiO2 powder itself was used under ambientcondition. Now both the reduction and oxidation sites are located on the TiO2 surface, andthe reduction of adsorbed oxygen molecules
proceeds on the TiO 2 surface. As alreadymentioned, the holes (h+) generated in TiO2
were highly oxidizing, and most compounds
were essentially oxidized completely, i.e., eachconstitution element of the compounds wasoxidized to its final oxidation state. In addition,
various forms of active oxygen, such as O2–,•
OH, HO2• and O•, produced by the following
processes may be responsible for the decomposition reactions.
e– + O2 → O2– (ad)O2–(ad) + H+ → HO2• (ad)h+ + H2O → •OH(ad) + H+
h+ + O2–(ad) → 2•O(ad)

(5)
(6)
(7)
(8)

For the purpose of easy handling ofphotocatalysts, the immobilization of TiO 2
powders on supports was carried out in thelate 1980s.19) Although many research studies
were on the purification of wastewater andpolluted air, TiO2 photocatalysis could not be
developed to the stage of a real industrial
technology in the 1980s.

4. TiO 2 Film Photocatalysis
under Weak UV Light in Early
1990s
In 1990, we carefully determined thereasons, in collaboration with TOTO Ltd., why
TiO2 photocatalysis could not be a practical��������
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Invited Review Paper

technology. We came to the conclusion that
it is fundamentally inadequate to utilize TiO2
photocatalysis for either energy acquisitionor the treatment of huge amounts of water
and/or air, because light energy density is
primarily low, and in addition, TiO2 can utilize
only the small amount of UV light contained insolar light. Based on such understanding, weconceived the idea of applying photocatalysis
targeting only the substances adsorbed originally on surfaces. In other words, we could
take the substances existing on two-dimensional surfaces as the object of decomposition
instead of those in three-dimensional spaces

Fig.4.

such as water or air. In this case, the absoluteamounts of the substances decrease, and thus,
the rather weak UV light existing in an ordinary environment could be a sufficient lightsource for maintaining the TiO2 surface clean.
We thus obtained the novel concept of lightcleaning materials, which would be coatedwith TiO2 film photocatalysts.20,21)

4.1 Photocatalytic cleaning effectof TiO2-coated materials
There exists typically several hundredµW/cm2 of UV light even in outdoor shade in

the daytime. This is low from the viewpoint ofenergy density, but corresponds to about 1015of photons/cm2 per second, which is a hugeamount compared to the number of molecules adsorbed on the surface. Let us consider,for example, a highly packed organic molecule monolayer. Figure 4 shows the atomic
force micrograph (AFM) images of monolayer stearic acid prepared on a TiO2 rutile(110) single crystal by the Langmuir–Blodgett
method. 22,23) The thickness of the organic
substance was about 2nm, and the number ofstearic molecules was roughly estimated to be
1016–1017/cm2. When this was exposed to UV

AFM images of monolayer of stearic acid on rutile (100) surface (1mW/cm2).

light of about 2.5mW/cm2, surface morphological changes were clearly observed, i.e.,
the inhomogeneous pitting of the film wasvery distinct. Further irradiation merged thepits, producing a mosaic that eventually disappeared with the progress of the reaction. After
20min, the island structure of the LB film was
no longer discernible, suggesting the complete
decomposition of stearic acid to CO2.
This observation suggests a potential utilization of the photocatalysis of TiO2-coatedmaterials, i.e., the surface coated with TiO2
could be kept clean. We first reported thistype of photocatalytic cleaning material witha ceramic tile in 1992.24) Heller et al. also
conceived a similar idea independently.25) Oneof the first commercialized products using
this effect was the self-cleaning cover glass
for tunnel light. In most tunnels in Japan,
sodium lamps emitting yellow light are used
for lighting, and the decrease in light intensity due to filming with exhaust compounds
is one of the most serious problems. A highpressure sodium lamp also emits UV light ofabout 3mW/cm 2 at a position of its coverglass. This UV light had not been consideredin the original purpose of the lighting, but issufficient to keep the surface clean when the
cover glass is coated with the TiO2 photocatalyst (Fig. 5).26) This light cleaning based on thephotocatalytic decomposition effect is used
now in other various commercial products
such as window blinds. However, it is important to note that this function is effective only
when the number of incident photons is muchgreater than that of filming molecules arriving on the surface perunit time. In other words, the function is not effective when the fluxof photons is insufficient comparedto that of the organic substances,even though the TiO2 photocatalyst is a very efficient one.

completely disappear on TiO2 after about one
week under a UV irradiation of 1mW/cm2. The
cell deactivation can be achieved in a much
shorter irradiation time, but still it takes nearly
1h under outdoor UV light intensity.27)
In contrast, the typical indoor UV lightintensity is about several hundred nW/cm2,
which is almost about three orders of magni-

4.2 Photocatalytic antibacterial effect of copperand/or silver-deposited
TiO2 film
A p h o t o c a t al y t i c d e c o m position reaction can be applicable to microorganisms. In fact,
Escherichia coli (E. coli ) cells can

Fig.5. Glass covers on highway tunnel lighting fixtures darkened byautomobile exhaust without TiO2 and maintained clean with TiO2.

JSAP International No.14 (July 2006)

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Fig.6. Changes in survival rate of copper-resistant E. coli cells on
Cu / TiO2 thin film. Error bars: standard deviations of three replicate experiments.

tude weaker than the outdoor one. Therefore,
the photocatalytic deactivation of microorganism requires a much longer time underindoor conditions than under outdoor ones;
thus, it cannot become a real practical technology. However, the anti-bacterial functionof a TiO2 photocatalyst is markedly enhanced
even with weak UV light, using a fluorescentlamp and the aid of either silver or copper,28)
which is harmless to the human body. Figure
6 shows the changes in the survival of copperresistant E. coli cells on a Cu-photodeposited
TiO 2 (Cu / TiO 2) film, indicating that E. coli
cells survived under dark conditions. However,when the Cu / TiO2 film is irradiated with very
weak UV light, the survival rate begins todecrease. This demonstrates photocatalytic
anti-bacterial activity even under weak UVlight obtained from indoor lighting from fluorescent light bulbs. The survival decay curves
under irradiation in Fig. 6 are not simple
exponential curves. Initial illumination had
a negligible effect on the survival rate, but
after 2 h, a marked decrease in survival wasobserved. We speculate that this cell deactivation proceeds as follows. The first step is thatthe reactive species generated by the TiO2
photocatalyst attacks the outer membrane[Fig. 7(b)]. The second step is the effective
uptake of the copper ions into the cytoplasmic
membrane [Fig. 7(c)]. In this case, the TiO2
photocatalytic reaction assists the intrusion of
the copper ions into the cell, which is probably why the E. coli cells are effectively killed
on a Cu / TiO2 film even under very weak UVlight.28) It has been reported that the copper

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JSAP International No.14 (July 2006)

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Fig.7. Schematic illustrations of bactericidal process for copper-resistant E. coli cells on Cu / TiO2 thin film
under weak UV light irradiation.

species photodeposited on the TiO2 film is a
mixture of metallic copper (Cu0) and copper
ions (Cu+ and Cu2+). When this Cu / TiO2 film
is irradiated, the copper ions can be reduced
to metallic copper and metallic copper can beoxidized to copper ions by photogenerated
electrons and holes, respectively. Although theoxidation state of copper might change under
UV light irradiation, copper ions (Cu2+) exist on
the Cu / TiO2 film.28) The enhancement of theantibacterial effect under weak UV light wasalso observed on the Ag-deposited TiO2. This
antibacterial technique is safe and effective.
It was observed that the number of bacteriaon the walls decreases to zero after installing
the photocatalytic tiles in an operating room.
In addition, the bacterial count in air was
also significantly decreased. The antibacterial
ceramic tile coated with photocatalytic TiO2
containing Cu and/or Ag started full-scale
manufacturing by TOTO Ltd. in 1995, and its
technology was exported to Western countries
widely.

5. Photo-induced Hydrophilicity
5.1 Water wettability of TiO2 surface
5.1.1 What is a photo-induced high hydrophilicity?
While investigating the novel concept oflight-cleaning materials coated with a TiO2
film photocatalyst under weak UV light in the
1990s, we have found in 1995 by chance themarked change in the water wettability of the

TiO2 surface before and after UV light irradiation. With the discovery of this phenomenon,
the application range of TiO2 coating has been
largely widen, as will be mentioned in detaillater.
The surface wettability is generally evaluated by the water contact angle (CA). The
CA (θ ) is defined as the angle between thesolid surface and the tangent line of the liquid
phase at the interface of the solid–liquid–gas
phases.
A TiO2 thin film exhibits an initial CA ofseveral tens of degrees depending on thesurface conditions mainly surface roughness.
When this surface is exposed to UV light,
water starts to exhibit a decreasing CA, that is,
it tends to spread out flat instead of beading
up.29,30) Finally, the CA reaches almost 0°, as
shown in Fig. 8(a). At this stage, the surface
becomes completely non-water-repellant andis termed ``highly hydrophilic’’. The surface
retains a CA of a few degrees for a day or two
under the ambient condition without being
exposed to UV light. Then, the CA slowly
increases, and the surface becomes the initialless hydrophilic state again, as shown in Fig.
8(b). At this point, the high hydrophilicity canbe recovered simply by exposing the surface
again to UV light. In short, this type of TiO2coated material is the only known practicalhighly hydrophilic one that shows stable andsemi permanent properties.
How can we explain this phenomenon?

Invited Review Paper

Just after applying oleic acid, both TiO2 andSrTiO3 surfaces were converted to the hydrophobic state with CAs of around 70° due tothe hydrophobic property of the oleic acidadsorbed on the surfaces. When UV light
was irradiated on the SrTiO3 surface, the CA
decreased to 20°, which was almost the sameas that observed before applying oleic acid. As
a result of conventional photocatalytic oxidation processes, surface-adsorbed oleic acidwas decomposed and almost removed, reproducing the initial surface. For the TiO2 surface,
however, the CA decreased to 0°, which was
lower than the initial value, showing that thehighly hydrophilic surface of TiO2 is not simply
attributed to the effect of the photocatalyticoxidation power.

UV

dark
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UV Irradiation Time/min
Fig.8.

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Dark Storage Time/hour

Changes in CA of TiO2 surface (a) under UV irradiation and (b) in the dark.

(ii) Relationship between amount of stains
and contact angle
We have vigorously attempted to find theanswer by analyzing it from various points ofview.29–31,35–37,39,44,45,48–50,53,54)

TiO2 is explained using a simple photocatalytic
decomposition mechanism.32–34) However, it
is important to note that a completely cleansurface cannot be obtained by the photocatalytic reaction because the surface is easily
contaminated by airborne stains under theambient condition. We have obtained many
experimental results showing that this highlyhydrophilic state is not a simple clean surface
but is a structurally changed metastable one.
Some of these results will be described below.

5.1.2 Characteristics of photo-induced highly hydrophilic state������ ��������
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(i) Comparison of hydrophilic properties ofTiO2 and SrTiO3 surfaces
Figure 9 shows the changes in CA
under UV light irradiation after applying oleic
acid to the surfaces of TiO 2 and SrTiO 3.35)

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Water contact angle / deg

First, we considered that this highly hydrophilic conversion originates from the cleansurface produced by the decomposition ofstaining compounds adsorbed on the surface
through the conventional photocatalyticoxidation. This is because metal oxides havelarge surface energies in general, and thus, weconsidered that a clean TiO2 surface could be
essentially hydrophilic. In fact, several reports
have recently been published, in which thephoto-produced highly hydrophilic state of

Figure 10 shows the representative theC 1s spectra of the TiO2 surface detected by
X-ray photoemission spectroscopy (XPS) before
and after UV light irradiations (60 min and12h). Before UV light irradiation, the carbon
peak derived from the stains was detected
and the CA on such surface was found to
be 56°. After 60min UV light irradiation, theCA was confirmed to be 0° when the distinct
carbon peak was detected, although theamount of stains decreased compared to that
before UV light irradiation. After further irradiation for 12h, the carbon peak still remained
and the CA was 0°. These experiments clearly
indicate that the highly hydrophilic conversion
can be completed even if stains remain on thesurface.

���Time / hourFig.9. Changes in water contact angle after applying oleic acid to surfaces ofTiO2 and SrTiO3.

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Fig.10. Change in XPS spectrum of TiO2 in C 1s peak region before and after
UV illumination with an intensity of 2.0mW/cm2.

JSAP International No.14 (July 2006)9������������������������

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Similarly, the highly hydrophilic state isturned to a less hydrophilic one by a ``wet
rubbing’’ method, which is a type of mechanochemical surface treatment with clean lint-free
paper. Kamei and Mitsuhashi reported that the
CA increases drastically from 3 to 80° by the
wet rubbing method.38) These results indicatethat the photo-produced highly hydrophilic
state is broken by external stimuli.

(iv) Temperature dependence of back reaction in the dark39)

When the highly hydrophilic TiO 2 film
prepared by UV light irradiation was sonicated in pure water, the CA was found toincrease to around 10°, as shown in Fig. 12.37)

As was described previously, the CA of
the photo-produced highly hydrophilic TiO2

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surface increases gradually toward the initialvalue in the dark even without any external
stimuli. However, the rate of this back reaction strongly depends on the ambient temperature. Figure 13 shows the result. Because
this measurement was carried out in a vessel
filled with synthetic air under the same conditions other than temperature, even if thesurfaces were adsorbed with stains, their influence could be ignored. It is obvious that theapparent rate was enhanced by increasing thetemperature. To estimate the activation energy
for this transformation, we used the rate (kb)obtained by the reciprocal plot of CA against
the logarithm of the dark storage time.31,40)
Figure 14 shows the natural logarithm of
kb obtained at CA of 20° versus the reciprocalof the absolute temperature. According to Fig.
14, the activation energy was calculated to be
62.4kJmol–1.

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Fig.12. Changes in water contact angle for TiO2 film subjected to alternate
ultrasonic treatment in pure water () and UV light irradiation ().

Subjected to cycles of alternating ultrasonictreatment and UV light irradiation, the watercontact angles switched between 0 and 10°
reversibly. It is hardly believed that the ultrasonic treatment makes the surface fouler.

(iii) Stability of photo-produced highly hydrophilic TiO2 surface���������

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Fig.11. Change in XPS spectrum of TiO2 in C 1s peak region before and afterrinsing in warm 4M NaOH solution (50ºC).

Figure 11 shows the changes in the C
1s XPS spectra before and after the treatment of the TiO2 surface in a warm concentrated NaOH solution. No distinct carbon
peak was detected within the experimental
error. Although the surface stains were nearlycompletely removed by this treatment, wefound that such a ``nearly clean’’ surface does
the CA of 20°, which is much higher thanthat of 0° induced by UV light.36) By considering these findings, only the removal of stains
cannot lead to the highly hydrophilic state
under the ambient condition.

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Fig.13. Ambient temperature dependence on less hydrophilic
conversion for TiO2 film maintained in the dark.

10

JSAP International No.14 (July 2006)

Fig.14. Activation energy of less hydrophilic conversion for TiO2 film kept in
the dark.

Invited Review Paper

5.1.3 Wettability of solid surface
Before examining some evidence forsurface structural changes accompanying thehighly hydrophilic conversion, let us briefly
review a classical theoretical treatment for
the wettability of the flat solid surface. It is
commonly evaluated in terms of the CA,
which is given by Young’s equation:41)

γ S =γ SL +γ L · cosθ ,(9)where γ S and γ L are the surface free energies
per unit area of the solid and liquid, respectively, and where γ SL is the interfacial freeenergy per unit area of the solid–liquid interface. In addition, γ SL can be approximatedusing the Girifalco–Good equation,42,43) with γ S
and γ L, asγ SL =γ S +γ L − Φ (γ S /γ L ) 1/2.

(10)cosθ = cγ S1/2–1 (c: constant).

(11)

This final equation shows that the CA
decreases simply with increasing γ S. Therefore,
it can be considered that the highly hydrophilic
state with a CA of 0° is achieved by the generation of some states with large surface energies when irradiated with UV light. As previously mentioned, the highly hydrophilic state
generated by UV light gradually returns to theinitial less hydrophilic state in the dark. Moreover, we showed that some external stimuli
and a higher ambient temperature increase
the rate of the back reaction. All these suggestthat the photo-produced state with a large
surface energy is metastable.

5.1.4 Structural changes on TiO2 surfaces irradiated with UV light(i) Domain formation after UV light irradiation
To gain information about surface changes
at the microscopic level, friction force microscopy (FEM) was utilized. A rutile TiO2(110)single crystal was used. Before UV light irradiation, no difference in contrast was observed,
indicating microscopically homogeneous wettability. After irradiation, the hydrophilic (bright)
and hydrophobic (dark) areas of 30–80nm wereclearly observed (Fig. 15).29) A gradual reversion to a smaller contrast was observed during
the storage of the crystal in the dark. In thisstudy, we concluded that the nanoscale separation between the hydrophilic and hydro-����������������

Here, Φ is a constant parameter ranging from
0.6 to 1.1, depending on the solid. In addition, γ L is the water surface free energy, which

has a constant value of 74mJ/m2. Therefore,by combining eqs. (9) and (10), the CA can be
simply expressed as

Fig.15. FFM images of rutile TiO2(110) single crystal surface before (left) and after (right)
UV light irradiation.

phobic phases accounts for the highly hydrophilic characteristic on the TiO2 surface.

(ii) Surface hardness change after UV lightirradiation
Hardness changes before and after irradiation with UV light on the surface of the rutileTiO2(110) single crystal were also observed.
Figure 16 shows the repetition of UV lighton and off dependence of surface hardness(within 50nm from the surface), inner hardness (300nm from the surface), and CAs.44)
When irradiated with UV light, CAs decreased
to 0°, accompanied by an increase in surface
hardness. In contrast, the inner hardness
remained constant. These findings suggested
that the highly hydrophilic surface is subjected
to compressive stress caused by the expansionof the surface volume.

5.1.5 What is the metastable state?
We have shown that the surface structureof TiO2 changes after UV irradiation, forming
a metastable state. Then, what is this state?
Thus far, we have not yet obtained a definite answer. However, several experimental
data indicate that the metastable state could
be caused by an increase in the number ofhydroxyl (OH) groups on the TiO2 surface.31)
This increase could be detected by X-ray
photoemission spectroscopy (XPS).36) The O
1s spectrum for the highly hydrophilic TiO2
surface exhibited a broad shoulder to thehigher binding energy side of the main O 1s
peak. The shoulder was fitted with two bands,
which are associated with the dissociatively

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Taking all the above experimental results
into consideration, we are certain that thephoto-produced TiO2 surface is not completely
clean but contains some stains, although it ishighly hydrophilic with a CA of almost 0°. In
other words, the removal of stains by oxidative decomposition can make the surface
only moderately hydrophilic, with a CA of
10–20° under the ambient condition. In addition, it seems that the highly hydrophilic state
is not the most stable state but forms somemetastable one. In fact, evidence has beenobtained, showing that the surface structureof TiO2 is changed by UV light irradiation,
which will be shown below.

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Fig.16. Relationship between changes in water contact angle and hardness at surface ofTiO2 film (within 50nm) and inside (300nm).

JSAP International No.14 (July 2006)11

adsorbed water on the TiO2 surface as well as
the physically adsorbed molecular water on
the dissociatively adsorbed OH groups. The
shoulder gradually decreased in size duringstorage in the dark. Therefore, these photogenerated surface OH groups were considered
to be thermodynamically metastable.

surface-enhanced IR absorption spectroscopy(SEIRAS).46)
Recently, Uosaki et al. reported thedifferences in interfacial water structures at
TiO2 surfaces between before and after UVlight irradiation by sum frequency generation (SFG) spectroscopy.47) It was shown thatUV light irradiation led to an increase in theamount of the ordered adsorbed water on
the TiO2 surface (a broad band with a peakat 3400cm–1 and a shoulder at 3200cm–1),
confirming the increase in the hydrophilicity ofthe surface.

Fourier transformation infrared (FTIR) spectroscopy provides another method of investigating the relationship between hydrophilicity
and the amount of OH groups.45) TiO2 showsIR bands positioned at 3695cm–1, assigned tothe stretching of OH groups chemisorbed on
the surface, 3300cm–1, assigned to hydroxyls
for both dissociated water and molecularly
adsorbed water, and 1623cm –1, pertaining
to H–O–H bending for molecular water. Thisobservation denotes the coexistence of dissociated water and molecular water on the TiO2
surface. Storage in the dark for one week
resulted in the decrease of all the bands,
correlated with both dissociated and molecularwater desorptions. The significant increase in
CA after the dark storage is consistent withthis surface conversion. The surface conversion is ascribed to the removal of the chemisorbed hydroxyl groups. With UV light irradiation, however, the intensity of the 1623cm–1
band decreased, whereas the 3695cm–1 band
increased, demonstrating the increase in theamount of adsorbed dissociated water andthe decrease in that of adsorbed molecularwater. Nakamura et al. also reported that theincrease in the amount of chemisorbed H2O
on the TiO 2 surface after UV light irradiation was observed (a band at 3270cm–1), by

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5.2 Application
On the basis of the previous studies
mentioned above and some electrochemical
experiments,48) which show that the photogenerated holes, not the electrons, areresponsible for the highly hydrophilic conversion, we proposed a mechanism for the highlyhydrophilic conversion under UV light irradiation, as shown in Fig. 17.31) That is, thephotogenerated holes produced in the bulkof TiO2 diffuse to the surface and are trappedat lattice oxygen sites. Most trapped holes are
consumed to react with the adsorbed organics
directly, or adsorbed water, producing OH radicals. However, a small portion of the trappedhole may react with TiO2 itself, breaking thebond between the lattice titanium and oxygenions by the coordination of water molecules at
the titanium site. The coordinated water molecules release a proton for charge compensa-

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The finding of the photo-induced hydrophilicity has markedly widened the application
range of TiO2-coated materials.49) That is, thestains adsorbed on the TiO2 surface can easily
be washed by water, because water soaks
between stain and the highly hydrophilic TiO2
surface. In other words, this has removed thelimitation of the cleaning function of the TiO2
photocatalysis, that is, the function is limitedby the number of photons. Even though thenumber of photons is not sufficient to decompose the adsorbed stains, the surface is maintained clean when water is supplied there.
Thus, the TiO 2-coated materials used
outdoors where they are exposed to rainfall

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Unstable OH(metastable state)hydrophilic

Fig.17. Schematic illustrations of reversible changes in amount of hydroxyl groups on TiO2
film under UV light irradiation and in the dark.

12

5.2.1 Self-cleaning function����������
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5.1.6 Mechanism for highly hydrophilic conversion

tion, and then a new OH group forms, leading
to the increase in the number of OH groups
at the surface. It is considered that the singly
coordinated new OH groups produced by UVlight irradiation are thermodynamically lessstable compared to the initial doubly coordinated OH groups. Therefore, the surface
energy of the TiO2 surface covered with thethermodynamically less stable OH groups ishigher than that of the TiO2 surface covered
with the initial OH groups. Because a water
droplet is substantially larger than the hydrophilic (or hydrophobic) domains, as shown in
Fig. 15, it instantaneously spreads completelyon such a surface, thereby resembling a
two-dimensional capillary phenomenon.

JSAP International No.14 (July 2006)

Fig.18. Conventional tent material (left) and TiO2-coated tent material (right).

Invited Review Paper

TiO2 that undergoes highly hydrophilic conversion has been required. We have intensively
investigated this on the basis of the mechanism for the highly hydrophilic conversion, as
described in §5.1.6.

Fig.19. Anti-fogging effect of automobile side-view mirror: conventional mirror (left) andTiO2-coated mirror (right).

5.2.2 Anti-fogging function
Another function blessed with the photoinduced hydrophilicity is the anti-fogging function. The fogging of the surfaces of mirrors
and glasses occurs when steam cools downon these surfaces to form many water droplets. On a highly hydrophilic surface, no water
drops are formed. Instead, a uniform thinfilm of water is formed on the surface. This
uniform water film prevents the fogging. Oncethe surface turns into the highly hydrophilic
state, it remains unchanged for several days or
one week. Thus, we expect that various glass
products, mirrors and eyeglasses, for example,
can be imparted with antifogging functions
using this technology, with simple processing
and at a low cost. In fact, Japanese-made cars
are being equipped with antifogging highlyhydrophilic side-view mirrors, as shown in Fig.
19.

6. Photocatalysis in 21st Century
As was described above, TiO2 photocatalysis has become a real practical technology
after the middle of the 1990s, particularly inthe field of building materials. It is, however,surprising that a research study on TiO2 photo-catalysis is still carried out for developing
both its science and technology after the 21st
century. In the following, some of the recent
development will be introduced.

6.1 Design of nanostructure of
TiO2 surface for highly sensitive hydrophilicity
When utilizing the photooxidative decomposition properties, TiO 2 has already been
applied to indoor use with the aid of either
copper or silver for anti-bacterial purpose, as
mentioned in §4.2. However, as for neither
the decomposition of VOC nor the utilizationof hydrophilic properties, TiO2 has yet to be
applied to indoor use. For example, the TiO2
surface does not undergo the highly hydrophilic conversion when the UV light has anintensity of 1µW/cm2, available in an ordinary
living environment. Thus, a highly sensitive

To obtain the appropriate faces, thephotoetching technique was applied to the(001) face of a rutile single crystal. As shownin the inset of Fig. 20, a large number of rectangular porous holes shaped like wells, witha size of 50–100nm, emerged with a fairly
regular arrangement. According to Sugiura
et al.51) and Nakato et al.,52) rectangular holes��������������������������

show a very effective self-cleaning function,i.e., stains are decomposed partially by theconventional photocatalytic reaction as well as
washed by rainwater. Such materials, which
we call ``photocatalytic building materials’’,e.g., exterior tiles, glass, aluminum walls, and
PVC fabric (Fig. 18), have already begun to becommercialized. For example, the photocatalytic exterior glass with an area of 20,000m2
was installed in the terminal building of Chubu
International Airport opened in 2005.

As the reconstruction of surface OH
groups is responsible for the hydrophilic
conversion, different types of hydrophilic
conversion behavior among the various single
crystal faces are expected to be observed bycomparing their surface atom alignments.
In fact, the (100) and (110) faces of a rutile
single crystal exhibited a higher hydrophilicity than the (001) face, as the former faces
have two-fold oxygens, which are higher inposition and energetically more reactive thantheir surrounding atoms and are so-called the``bridging site oxygens’’, whereas the latter has
three-fold oxygens, which are lower in position and energetically more inactive.50) Therefore, the (100) and (110) faces are favorable
for increasing the number of OH groups. Thisfinding could serve as a guideline for selecting
the appropriate faces of the TiO2 crystal forsurface exposure.

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Fig.20. Changes in water contact angles on rutile (001) surface with and without
photoetching treatments. The inset shows a SEM image of rectangular holes emerged byphotoetching treatment on a (001) surface.

JSAP International No.14 (July 2006)13

proceed toward the 〈001〉 direction (c -axis
direction), and the (100) face or equivalents
are exposed selectively on the walls. This rectangular porous surface increased the sensitivityof the photoinduced hydrophilic reaction andachieved a high hydrophilicity under UV lightirradiation of 1µW/cm2, whereas the surface
without a photoetching treatment did not,as shown in Fig. 20.53) Because the surface
roughness enhances the hydrophilicity, thehigh sensitization for hydrophilic conversion
by the photoetching treatment was causedby the exposure of faces with bridging siteoxygens and the increase in surface roughness. This high sensitization was also observedon the rutile polycrystal by the photoetchingtreatment, which suggested that this technique is applicable to anatase thin films.

regardless of the residual stresses. The surface
morphologies of the four films were controlled
to be the same, and therefore, the residual
stress is an important factor influencing thehighly sensitive photoinduced hydrophilicity ofa film.
The other highly sensitive system weproduced is the heterogeneous TiO 2/WO 3
one.55) As photogenerated holes are effectively
accumulated on TiO2 without recombining
with electrons, and as WO 3 could absorb
visible light contained in the fluorescent lightup to a wavelength of around 440nm due
to its bandgap of 2.8eV, the reaction responsible for the increased hydrophilicity was
greatly enhanced, and the high hydrophilicity
was achieved on this system irradiated withextremely weak UV light with an intensity of
1µW/cm2 from a fluorescent lamp. As such,the high sensitization of TiO2 under weak UVlight is expected to increase the application
areas to indoor conditions.

The introduction of residual tensile stress toanatase thin films is also a candidate method
to increase the sensitivity. As the hydrophilic
conversion is caused by the increase in thenumber of surface OH groups, the Ti–O bondlength should be larger in the highly hydrophilic surface than in the less hydrophilic
surface. In fact, as previously mentioned, thesurface volume increased after UV light irradiation. Therefore, it can be expected that theTiO2 surface in the presence of tensile stressis favorable for hydrophilic conversion. The
residual tensile stress in the anatase thin film
fabricated by the sputtering technique greatly
enhanced the hydrophilic behavior, compared
to a thin film without residual stress, as shownin Fig. 21.54) In contrast, the compressive stressdegraded the hydrophilic behavior. The photocatalytic oxidation activities were identical

6.2 Visible-light-sensitive TiO2
The current area of interest in this fieldhas been the modification of TiO2 sensitive
to visible light. One approach was to substitute Cr, Fe or Ni for a Ti site.56,57) Anotherapproach was to form Ti3+ sites by introducing
an oxygen vacancy in TiO2.58) However, theseapproaches were not widely accepted dueto the lack of reproducibility and chemical
stability.
In 2001, several groups reported visiblelight-sensitive TiO2-based powders and thin��������������
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Fig.21. Changes in water contact angles on TiO2 films when irradiated with
UV light, without residual stress and with residual tensile/compressive stresses.

14

JSAP International No.14 (July 2006)

films.59–61) Subsequently, nitrogen-doped TiO2
has attracted considerable attention.62–64) In
fact, similar photocatalysts sensitive to visible
light have already been reported in 1986.65,66)
Yellow and transparent nitrogen-doped
TiO2 thin films can be fabricated by sputteringa Ti or TiO2 target in a gas flow that contains
N2O or N2.61) The N 1s XPS peak at 396eV indicates that the dopant nitrogen is located at anoxygen site.60,61)
Figure 22(a) shows the hydrophilic
conversion behaviors of the nitrogen-doped
TiO 2 thin film irradiated with visible light(400–530nm). The nitrogen-doped TiO 2
thin film underwent hydrophilic conversion;
however, irradiating only with visible light did
not achieve the high hydrophilicity. Irradiatingwith UV light (300–400nm), the nitrogendoped TiO2 thin film underwent highly hydrophilic conversion, as shown in Fig. 22(b).
The photocatalytic activities (both oxidative
decomposition and hydrophilic conversion
activities) generated by visible light-induced
holes are inferior to those generated by UVlight-induced ones.67)
Before discussing the reason for this, let
us discuss the origin of visible light sensitivity.
When the N atoms are substituted as N 3–
ions at O2– sites, the impurity (accepter) level,composed of 2p orbitals of N (N 2p), is formed
above the valence band. Electron vacancies
exist at the acceptor level. Therefore, nitrogendoped TiO2 should be a p-type semiconductor
as electrons are thermally excited from thevalence band. However, we have photoelectrochemically and electrochemically determined that the nitrogen-doped TiO2 was ann-type semiconductor and the carrier concentration increased as the dopant concentration
increased. Actual TiO2 is known to be nonstoichiometric and have oxygen defects. Oxygen
defects generate electrons, which leads to then-type semiconductor. The amount of electrons, originated from oxygen vacancies, isconsidered to be larger than that of electron
vacancies, originated from the nitrogen substitution at O sites. Therefore, the nitrogendoped TiO 2 should be an n-type semiconductor. Thus, with increasing dopant nitrogen,the carrier concentrations should decrease.
However, the experimental results are theopposite. When nitrogen is incorporated,because an increase in the amount of intersti-

Invited Review Paper

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Fig.22. Changes in water contact angles on TiO2 and nitrogen-doped TiO2 thin films irradiated with (a) vis and (b) UV lights.

tial titanium is clearly not possible, an oxygen
vacancy is simultaneously produced. Therefore, the schematic illustration in Fig. 23 is theessential procedure when oxygen is replacedby nitrogen.
The Ti 3d impurity (donor) level, derived
from oxygen vacancies, is known to be nonvisible light sensitive. In fact, hydrogen-reduced
TiO2 (TiO2-x) powders, which have a gray color,
do not show visible light sensitivity. The N 2p
level exists much deeper than the Ti 3d donor
level, from which we can consider that the N
2p level has a much more oxidation power
than the Ti 3d level. Therefore, the origin ofvisible light sensitivity of nitrogen-doped TiO2
is considered to be the N 2p narrow band.
Thus, the reason that irradiating thenitrogen-doped TiO2 with UV light resulted inhigher photocatalytic activities than irradiatingwith visible light is as follows. Irradiating with
UV light excites electrons in both the valenceband composed of O 2p and the narrow band
composed of N 2p, but irradiating with visible
light only excites electrons in the narrow bandof N 2p. In addition, the hole mobility in theisolated narrow band should be low. Therefore, the hydrophilic properties when irradiating with UV light were higher than whenirradiating with visible light. Although thenitrogen concentration increases, it is notsuggested by the density of states (DOS) calculations that the bandgap narrowing by mixing
N 2p with O 2p occurs.

These anion-doped TiO 2 are candidate
photocatalysts in terms of reproducibility andchemical stability. Therefore, further researchand practical applications are desirable.

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�����will show the higher photocatalytic activities
irradiated with visible light. This investigation is
now under way.72)

Compared with the conventional TiO2,
the advantage of nitrogen-doped TiO2 is theincreased absorbed photon number, but thedisadvantage is the decreased photocatalytic
activity. Therefore, whether to use nitrogendoped TiO2 or conventional TiO2 depends on
the light source.

As the discovery of the photo-inducedhydrophilicity has markedly widened the application field of TiO2-coated materials, a highlyhydrophobic TiO2 surface could open a new
application field. In addition, if it is realized,
we will be able to control the wettability on
a TiO2 surface using external stimuli, such as
UV light, which we believe is both scientificallyand practically very important.
Let us try to design the hydrophobic TiO2
surface. As previously mentioned, the wettability of a flat solid surface is determined
simply by the surface free energy of solid as
described in eqs. (9) and (11). As for a non-flat
surface, however, surface roughness affects
the wettability. Wenzel modified Young’s
equation by considering the surface roughness
to obtain73)

In addition to nitrogen, the sulfur-doped
and carbon-doped TiO2 systems are reported
to be visible-light-sensitive photocatalysts.68–71)
cosθ ’ = r cosθ ,(12)However, the visible-light-induced photocatalytic activities of these anion-doped TiO2 arewhere θ ’ is the apparent contact angle andinsufficient and should be further enhanced.
r is the surface roughness ratio between theThis is because the introduced 3p
orbitals of S (S 3p) and 2p orbitalsof C (C 2p), similar to N 2p, also������formed the localized narrow band
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compared with the isolated one,

JSAP International No.14 (July 2006)

15

nating between UV light and dark storage.75)
At present, the hydrophobic conversion takes
much time, and must be further enhanced.

Fig.24. SEM images for polycrystalline TiO2 surfaces (a) before and (b) after etching treatments.

actual surface area and the apparent surface
area. This equation indicates that the surface
roughness enhances the hydrophilicity ofhydrophilic surfaces (θ <90°) and also enhances
the hydrophobicity of hydrophobic surfaces(θ >90°) since the r value is always larger than 1.
Because the CA of a flat TiO2 surface is always
less than 90°, the hydrophobic TiO2 surface
cannot be obtained by considering only the
Wenzel equation. To realize the hydrophobic
TiO2 surface, we must introduce a different
concept to describe the CA (θ ’) on a roughsurface. Cassie proposed an equation for asurface composed of solid and gas.74) Whena unit area of the surface has an area friction,f, where a water droplet contacts the solid
surface with a CA of θ , the θ ’ on the surface
can be expressed as follows, called Cassie’s
equation, in which the CA for air is assumed
to be 180°:

at room temperature in a clean vessel filledwith synthetic air. Maintaining the samples inthe dark for 15 days caused the CA to reachapproximately 120° on the etched surface,whereas the CA was around 80° on thenonetched surface, indicating that we could
obtain the hydrophobic TiO2 surface, on which
Cassie’s mode dominates, by the photoetchingprocess (Fig. 25).
The UV irradiation of this hydrophobic
TiO2 markedly changed the surface wettability, i.e., the CA decreased to 0°. In addition, storing the samples in the dark for a longtime caused the CA on the etched surface
to further increase to approximately 140°,
whereas the CA on the nonetched surface
remained constant at around 80°. We canthus control the surface wettability from highlyhydrophilic to hydrophobic repeatedly by alter-

In addition, the surface with a CA above
150° is called the super-hydrophobic surface,and such a surface is attracting considerable
attention at present,76–84) because the limited
contact area between the solid surface andthe water could change chemical reactions
and/or bond formation through water, introducing novel properties on the surface. Therefore, if one succeeds in the preparation of the
TiO2 surface with a CA of more than 150°, it
indicates that the surface property of TiO2 canbe markedly controlled.

6.4 New environmental applications
TiO2-coated materials practically used thus
far have been provided with self-cleaning, antibacterial and/or anti-fogging functions basedon the photo-induced decomposition reaction
and photo-induced hydrophilicity. It is important to note that these functions are obtained
without using any chemicals, but with only
sunlight and rainwater. Therefore, these TiO2coated materials can be classified as being
environmentally friendly. In this section, we
will show further applications of TiO2 photocatalysis, which can actively contribute to environmental preservation and/or improvement
technologies.

cosθ ’ = f cosθ + (1– f )cos 180°
(13)

Considering eq. (13), the θ ’ increases withdecreasing f value. Thus, the hydrophobic
TiO2 requires surface roughness where air can
intrude between the water droplet and theTiO2 surface.
To achieve such a rough surface, weapplied a photoetching technique to a rutile
pellet. Before the etching treatment, grains
and grain boundaries were observed, which
is typical of a polycrystalline pellet, as shownin Fig. 24(a). After etching, the surface structure changed and was accompanied by anincrease in surface roughness. Random directions of digging ``ditches’’ as shown in Fig.
24(b) were plausible, considering the polycrystalline pellet. The pellets with the etched andnon-etched surfaces were stored in the dark

16

JSAP International No.14 (July 2006)�����������������������

= f cosθ + f –1.

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Fig.25. Back reactions on etched and nonetched polycrystalline TiO2 surfaces as afunction of storage time in the dark.

Invited Review Paper

6.4.1 Photocatalytic decomposition of pollutants
Environment pollution, including water,
air and soil is becoming an increasingly serious
problem today. There have been many reports
aiming at applying TiO2 photocatalysis to pollution clean-up since the 1970s. However, thepurification of the three-dimensional spaces byphotocatalysis is much more difficult than thatof the two-dimensional surface of building
materials due to the following two reasons.
One is that photocatalytic reactions are
surface reactions and thus the reactants must
be captured by the photocatalyst surface. The
other is that the total amount of reactant is,in general, higher in three-dimensional spaces
than on a two-dimensional surface, indicatingthat much more light energy is necessary
for the purification of the three-dimensional
space. Therefore, practical technologies havenot been obtained in this field. However, wehave recently succeeded in the construction ofpractical purification systems for wastewaterfrom agriculture and soil polluted by volatileorganic compounds (VOCs). These systems
are based on TiO2 photocatalysts and use only
solar light.
Important keys for these successes are(1) the utilization of nanosized TiO2 photocatalyst powders dispersed on substrates
with extremely large surface areas, and (2)spreading them on the ground widely tocollect sunlight. Because the concentrations ofenvironmental pollutants are low in general,
the UV light contained in sunlight is sufficiently
strong to decompose them by TiO2 photocatalysis, if we can collect the light from a broad
area.

large surface area deposited with very photoactive TiO2 nanoparticles; we were able toshow that the wastewater solution is easily
purified using the photocatalytic mat under
only solar light. The treatment method isvery simple, i.e., the wastewater is poured
onto mats that are spread over a wide areaon the ground. The agricultural chemicals
were completely decomposed under sunlightin a few days. It is surprising that the initial
total organic carbon (TOC) values of several
hundred to one thousand ppm decreased tonearly zero in one week. This could be one of
the simplest and easiest environmental technologies.

in Fig. 26. The wastewater from the hydroponic tomato culture with a planting area of
about 80m2 was introduced into a shallow
vessel with a bottom area of 4m2 and a depthof 10cm in which porous ceramic plates
coated with TiO 2 photocatalyst nanoparticles were placed. The organic contaminantsin the wastewater were easily decomposed
under solar light, but the nutrient compounds
containing nitrogen, phosphorous and potassium were not, because these components
existed in their most oxidized forms, NO3–,
PO43– and K+, in the nutrient solution. Therefore, this system is also expected to serve as anutrient-saving technology.

(ii) Water treatment of hydroponic culture
system(iii) Treatment of VOC-polluted soil

Most of the hydroponic culture installations are adopting run-to-waste systems (asopposed to recirculating). The nutrient solution contains highly concentrated nitrogen andphosphorus compounds, and thus, the wastewater causes soil pollution. From the viewpoint of environmental problems, the recyclingof nutrient solutions is desirable. However,organic contaminants accumulate in the solution, inhibiting plant growth.
We succeeded in constructing a recycling system in a tomato hydroponic culture
system using the TiO2 photocatalyst and solar
light. The system is schematically illustrated(i) Detoxification of wastewater used forrice hull disinfection
Disinfection solutions for rice hulls (to stop
the spread of plant diseases) contain highly
concentrated agricultural chemicals. The corresponding wastewater is mostly disposed of by
pouring onto the ground, which causes soil
pollution. The amount of wastewater from ricehull disinfection amounts to about 500,000
metric tons/year in Japan, for example. Sucha problem could also become much more
serious in developing countries.

Volatile chlorinated organic compounds(VOCs), such as trichloroethylene and tetrachloroethylene, have been widely used assolvents for the dry cleaning of clothes andwashing of semiconductors. They had been
indiscriminately disposed by the middle of the
1980s, causing soil and groundwater pollution. These types of pollution are serious environmental problems, because the carcinogenic
and toxic chemicals had been widely disposed.
The most common method of treating thepolluted soil is either the simple replacementwith clean soil or the heating of the soil tovolatilize the VOCs into air. It is obvious thatthese methods do not truly purify the environment.

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Fig.26. Novel photocatalytic water recycling system of tomato hydroponic culture.

We developed a glass wool mat with a

JSAP International No.14 (July 2006)17

We designed photocatalytic sheets topurify the polluted soil on the ground using
sunlight. As shown in Fig. 27, the polluted soil
is dug up and covered with the sheet, which
is made of corrugated paper containing both
TiO2 powder adsorbed on activated carbon
powders. Then the covered soil is heated (forexample, by mixing with calcium oxide), volatilizing the pollutant gases captured by adsorption on activated carbon incorporated in the
sheet material. The sheet is allowed to remain
undisturbed under sunlight, while TiO2 in the
sheet decomposes the pollutants completelyby photocatalytic reaction. We have examined the efficacy of this method at an actual
polluted field and confirmed that the VOCs
became completely harmless after several
weeks. This purification method could be oneof the real environmental purification technologies.

surface area of water. Thus, the cultivation ofrooftop plants and / or the construction of artificial lakes or marshes are currently under way.
However, the areas of green tract land andwater surfaces cannot be secured easily due tothe high land value in urban areas.

6.4.2 Efficient water evaporation from hydrophilic surfaces

It is important to emphasize that thebuildings and surroundings are not cooled bywater itself, but by the latent heat flux whenwater evaporates. In fact, it is often observedthat the temperature of a wall surface is lower
than that of sprinkling water. The thinner
the water layer is, the more effectively thebuilding surface temperature and surrounding
air temperature decrease as the amountof latent heat flux decreases to cool down
the thin water film. Although the margin of
the temperature drop depends on the color
and / or type of building material, as well as
the atmosphere temperature and humidity, it

Rapid increases in the absorption of solar
energy and increases in energy consumption
in large cities cause a temperature increase,the so-called heat island phenomenon. The
former is due to the coverage of the groundsurface by artificial structures, such as buildings and paved roads, and the latter is dueto the heat emissions from automobile traffic
and air conditioners. An effective method of
preventing the heat island phenomenon isincreasing the area of green tract land or the

We are proposing a method of securing
water surfaces by continuously sprinklingwater onto the surfaces of buildings that will
be covered with a TiO2 photocatalyst (Fig.
28). The surface coated with TiO2 becomes
highly hydrophilic and plays an importantrole in minimizing the amount of sprinklingwater required to form a water film. A verythin water layer of approximately 0.1mm
thickness can cover all of the highly hydrophilic TiO2 material; the water can be continuously supplied in small quantities for a verticalbuilding.

was confirmed on a clear day in the middleof summer that the temperature drops were
15ºC on window glass and 40–50ºC on black
roof-tile surfaces. Moist surfaces easily mildew,
but since a TiO2 photocatalyst has oxidation
activity in addition to a high hydrophilicity, thisproblem is not an issue.
The cooling of the building surface also
results in the reduction in the amount of electricity consumed for air conditioning. We
measure this effect quantitatively with a realhouse and building and observe that theamount of electricity consumed is reduced by
ten to several tens of percentage. Therefore,
TiO2-coated materials could also contribute to
the development of energy-saving technologies.

7. Conclusions
In this paper, an overview of the development of TiO2 photocatalysis and its future
prospects from both scientific and technological viewpoints are given. It is interesting
to note that this field has experienced major
developments every ten years for the last
thirty years, namely, water photoelectrolysis(Honda–Fujishima effect) in the early 1970s,
photocatalytic H2 production in the 1980s, andthe photocatalysis and hydrophilicity of TiO2
films in the 1990s. Based on the basic research
results, real industrial applications have beenachieved since the end of the 1990s. In addition, this field is still being developed further inthe 21st century. We believe that TiO2 photocatalysis is one of the best examples how, on
the time scale of tens of years, basic scientificknowledge can be developed into a technological field and can produce a new industry.

Acknowledgment�������������������� ��������� �����

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��������

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Fig.27. Purification system for polluted soil utilizing solar energy and photocatalyst sheets.

18

JSAP International No.14 (July 2006)

The authors gratefully thank many collaborators in both academia and industry who
have been involved in the present research.
We also thank Dr. D. A. Tryk for carefully
reading the manuscript.

Invited Review Paper

Continuous sprinkling water onto
TiO2-coated surfaces

Latent heat flux bywater evaporation

Rainwater reservoir

1 ) E. Keidel: Farben-Zeitung. 34 (1929) 1242.
2 ) C. F. Doodeve and J. A. Kitchener: Trans. Faraday Soc. 34 (1938) 902.
3 ) For example, S. Kato and F. Mashio: Abtr. Book
Annu. Meet. Chemical Society of Japan, 1956,
p.223.
4 ) S. Kat and F. Masuo: Kogyo Kagaku Zasshi 67(1964) 1136 [in Japanese].
5 ) A. Fujishima, K. Honda and S. Kikuchi: Kogyo
Kagaku Zasshi 72 (1969) 108 [in Japanese].
6 ) A. Fujishima and K. Honda: Nature 238 (1972)37.
7 ) W. Jaegermann: in The Semiconductor/
Electrolyte Interface: A Surface Science Approach, eds. R. E. White, B. E. Conway, J. O’M.
Bochris (Plenum Press, New York, 1996) Modern Aspects of Electrochemistry, Vol.30, p.1.
8 ) A. J. Nozik and R. Memming: J. Phys. Chem.
100 (1996) 13061.
9 ) A. Fujishima and D. A. Tryk: in Photoelectrochemical Conversion, ed. K. Honda (Springer,
Tokyo, 1999) Functionality of Molecular Systems, Vol.2, p.196.
10 ) N. Sato: Electrochemistry at Metal and Semiconductor Electrodes (Elsevier, Amsterdam,
1998).
11 ) L. M. Peter: in Photoelectrochemical Kinetics at
Semiconductor Electrodes, eds. R. G. Compton
and G. Hancock (Elsevier, Amsterdam, 1999)
Applications of Kinetic Modeling, Vol.37, p.223.
12 ) M. K. Nazeeruddin, A. Kay, I. Rodicio, R.
Humphry-Baker, E. Mueller, P. Liska, N. Vlachopoulos and M. Gräzel: J. Am. Chem. Soc. 115(1993) 6382.
13 ) M. K. Nazeeruddin, P. Pechy and M. Gräzel:Chem. Commun. 18 (1997) 1705.

14 ) This field remains active, with novel layered
metal oxides being the favored materials. For
example, a very efficient production of H2 andO2 using deep UV light of around 290nm has
been reported.
15 ) T. Kawai and T. Sakata: Nature 286 (1980) 474.
16 ) L. Kavan, M. Gräzel, S. E. Gilbert, C. Klemenz
and H. J. Scheel: J. Am. Chem. Soc. 118 (1996)
6716.
17 ) S. N. Frank and A. J. Bard: J. Am. Chem. Soc. 99(1977) 303.
18 ) Many reviews have been published. For example, M. A. Fox and M. T. Dulay: Chem. Rev.
93 (1993) 341; M. R. Hoffman, S. T. Martin, W.
Choi and D. W. Bahnemann: Chem. Rev. 95(1995) 69.
19 ) R. W. Matthews: J. Phys. Chem. 91 (1987)
3328.
20 ) T. Watanabe, K. Hashimoto and A. Fujishima:
in Photocatalytic Purification and Treatment of
Water and Air, eds. D. F. Ollis and H. Al-Ekabi(Elsevier, Amsterdam, 1993).
21 ) A. Fujishima, K. Hashimoto and T. Watanabe:
TiO2 Photocatalysis: Fundamentals and Applications (BKC, Tokyo, 1999).
22 ) P. Sawunyama, L. Jiang, A. Fujishima and K.
Hashimoto: J. Phys. Chem. B 101 (1997) 11000.
23 ) P. Sawunyama, A. Fujishima and K. Hashimoto:Langmuir 15 (1999) 3551.
24 ) T. Watanabe, K. Hashimoto and A. Fujishima:
Proc. 1st Int. Conf. TiO2 Photocatalyst, ed. H. AlEkabi, 1992.
25 ) A. Heller: Acc. Chem. Res. 28 (1995) 503.
26 ) H. Honda, A. Ishizaki, R. Soma, K. Hashimotoand A. Fujishima: J. Illum. Eng. Soc. (1998) 42.
27 ) K. Sunada, Y. Kikuchi, K. Hashimoto and A. Fujishima: Environ. Sci. Technol. 32 (1998) 726.

Fig.28. Energy-saving system using
solar light and stored rainwater.

28 ) K. Sunada, T. Watanabe and K. Hashimoto: Environ. Sci. Technol. 37 (2003) 4785.
29 ) R. Wang, K. Hashimoto, A. Fujishima, M. Chikuni, E. Kojima, A. Kitamura, M. Shimohigoshi andT. Watanabe: Nature 388 (1997) 431.
30 ) R. Wang, K. Hashimoto, A. Fujishima, M. Chikuni, E. Kojima, A. Kitamura, M. Shimohigoshi andT. Watanabe: Adv. Mater. 10 (1998) 135.
31 ) N. Sakai, A. Fujishima, T. Watanabe and K.
Hashimoto: J. Phys. Chem. B 107 (2003) 1028.
32 ) J. M. White, J. Szanyi and M. A. Henderson: J.
Phys. Chem. B 107 (2003) 9029.
33 ) C. Wang, H. Groenzin and M. J. Schltz: Langmuir 19 (2003) 7330.
34 ) T. Zubkov, D. Stahl, T. L. Thompson, D. Panayotov, O. Diwald and J. T. Yates, Jr.: J. Phys. Chem.
B 109 (2005) 15454.
35 ) M. Miyauchi, A. Nakajima, A. Fujishima, K.
Hashimoto and T. Watanabe: Chem. Mater. 12(2000) 3.
36 ) R. D. Sun, A. Nakajima, A. Fujishim, T. Watanabe and K. Hashimoto: J. Phys. Chem. B 105(2001) 1984.
37 ) N. Sakai, R. Wang, A. Fujishima, T. Watanabe
and K. Hashimoto: Langmuir 14 (1998) 5918.
38 ) M. Kamei and T. Mitsuhashi: Surf. Sci. 463(2000) L609.
39 ) H. Irie, M. S. Utami, T. Shibata and K. Hashimoto: submitted to Chem. Commun.
40) kb was obtained using θ and t described as the
CA and dark storage time (min), respectively.
1/θ = a – b×ln(t)d(1/θ ) / dt = –b×(1/t)
Combining these equations, kb can be
described as a function of 1/θ :kb(deg–1·min–1) = –d (1/θ ) /dt = b ×exp ( (1/θ –a)/b).

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Invited Review Paper41 ) Principles of Colloid and Surface Chemistry, ed.
P. C. Hiemenz (Dekker, New York, 1986) p.307.
42) L. A. Girifalco and R. J. Good: J. Phys. Chem. 61(1957) 904.
43) R. J. Good and E. Elbing: Ind. Eng. Chem. 62(1970) 54.
44) T. Shibata, H. Irie and K. Hashimoto: submitted
to J. Phys. Chem. B.
45) K. Hashimoto and T. Watanabe: Hyomen
Kagaku 20 (1999) 27 [in Japanese].
46) R. Nakamura, K. Ueda and S. Sato: Langmuir 17(2001) 2298.
47) K. Uosaki, T. Yano and S. Nihonyanagi: J. Phys.
Chem. B 108 (2004) 19086.
48) N. Sakai, A. Fujishima, T. Watanabe and K.
Hashimoto: J. Phys. Chem. B 105 (2001) 3023.
49) A. Fujishima, K. Hashimoto and T. Watanabe:
TiO2 Photocatalysis, Fundamentals and Applications (BKC, Tokyo, 1999).
50 ) R. Wang, N. Sakai, A. Fujishima, T. Watanabe
and K. Hashimoto: J. Phys. Chem. B 103 (1999)
2188.
51 ) T. Sugiura, T. Yoshida and H. Minoura: Electrochemistry 67 (1999) 1234.
52 ) A. Tsujiko, T. Kisumi, Y. Magari, K. Murakoshi and
Y. Nakato: J. Phys. Chem. B 104 (2000) 4873.
53 ) T. Shibata, T. Watanabe, K. Hashimoto and A.
Nakajima: Photocatalysis 4 (2001) 45 [in Japanese].
54 ) T. Shibata, H. Irie and K. Hashimoto: J. Phys.
Chem. B 107 (2003) 10696.
55 ) M. Miyauchi, A. Nakajima, K. Hashimoto and T.
Watanabe: Adv. Mater. 12 (2000) 1923.

56 ) E. Borgarello, J. Kiwi, M. Gratzel, E. Pelizzetti
and M. Visca: J. Am. Chem. Soc. 104 (1982)
2996.
57 ) H. Yamashita, Y. Ichihashi, M. Takeuchi, S. Kishiguchi and M. Anpo: J. Synchrotron Radiat. 6(1999) 451.
58 ) I. Nakamura, N. Negishi, S. Kutsuna, T. Ihara,
S. Sugihara and K. Takeuchi: J. Mol. Catal. 161(2000) 205.
59 ) Y. Sakatani, K. Okusako, H. Koike and H. Ando:
Photocatalysis 4 (2001) 51 [in Japanese].
60 ) T. Ihara, M. Ando and S. Sugihara: Photocatalysis 5 (2001) 19 [in Japanese].
61 ) R. Asahi, T. Ohwaki, K. Aoki and Y. Taga: Science 293 (2001) 269.
62 ) H. Irie, Y. Watanabe and K. Hashimoto: J. Phys.
Chem. B 107 (2003) 5483.
63 ) H. Irie, S. Washizuka, N. Yoshino and K. Hashimoto: Chem. Commun. 11 (2003) 1298.
64) S. Sakthivel and H. Kisch: Chem. Phys. Chem. 4(2003) 487.
65 ) S. Sato: Chem. Phys. Lett. 123 (1986) 126.
66 ) H. Noda, K. Oikawa, T. Ogata, K. Matsuki and H.
Kamada: Nippon Kagaku Kaishi (1986) 1084 [inJapanese].
67 ) H. Irie, S. Washizuka, Y. Watanabe, T. Kako and
K. Hashimoto: J. Electrochem. Soc. 152 (2005)
E351.
68 ) T. Umebayashi, T. Yamaki, H. Itoh and K. Asai:
Appl. Phys. Lett. 81 (2002) 454.
69 ) T. Umebayashi, T. Yamaki, S. Tanaka and K. Asai:
Chem. Lett. 32 (2003) 330.

70 ) T. Ohno, T. Mitsui and M. Matsumura: Chem.
Lett. 32 (2003) 364.
71 ) H. Irie, Y. Watanabe and K. Hashimoto: Chem.
Lett. 32 (2003) 772.
72 ) H. Irie and K. Hashimoto: Photocatalysis 15(2004) 78 [in Japanese].
73 ) R. N. Wenzel: J. Phys. Colloid Chem. 53 (1949)
1466.
74 ) A. B. D. Cassie: Discuss. Faraday Soc. 3 (1948)11.
75 ) H. Irie, T. S. Ping, T. Shibata and K. Hashimoto:Electrochem. Solid-State Lett. 8 (2005) D23.
76 ) A. Nakajima, K. Hashimoto and T. Watanabe:
Monatsh. Chem. 132 (2001) 31.
77 ) A. Nakajima, A. Fujishima, K. Hashimoto and T.
Watanabe: Adv. Mater. 11 (1999) 1365.
78 ) A. Nakajima, K. Abe, K. Hashimoto and T.
Watanabe: Thin Solid Films 376 (2000) 140.
79 ) A. Nakajima, K. Hashimoto, T. Watanabe, K.
Takai, G. Yamauchi and A. Fujishima: Langmuir
16 (2000) 7044.
80 ) N. Ogawa, M. Soga, Y. Takada and I. Nakayama: Jpn. J. Appl. Phys. 32 (1993) L614.
81 ) K. Tadanaga, N. Katata and T. Minami: J. Am.
Ceram. Soc. 80 (1997) 1040.
82 ) K. Tadanaga, N. Katata and T. Minami: J. Am.
Ceram. Soc. 80 (1997) 3213.
83 ) A. Hozumi and O. Takai: Thin Solid Films 303(1997) 222.
84) A. Hozumi and O. Takai: Thin Solid Films 334(1997) 54.

Kazuhito Hashimotostudied Chemistry at the
University of Tokyo and received his B.S., M.S., and
Ph. D. degrees in 1978,
1980, and 1985, respectively. From 1980 till 1989,
he served at Institute for
Molecular Science as atechnical associate and a
research associate. He joined the University of Tokyo as
a lecturer in 1989. He became an associate professor at
the University of Tokyo from 1991 and was promoted toa full professor in 1997. He served as a director of Photochemical Conversion Project at Kanagawa Academyof Science and Technology from 1994 till 1999, and has
been a group leader of Research Laboratory for Optical Science at the same Academy from 1999 till now. At
present, he is the Director General of Research Center
for Advanced Science and Technology (RCAST) at the
University of Tokyo. Also, he is a professor of RCAST and
Department of Applied Chemistry at the same University concurrently. He has received several awards for his
research excellence from various societies, such as theJapan Lightings Society, the Photochemical Society of Japan, and the Electrochemical Society of Japan. Also, he
received the IBM Science Award from IBM Science Foundation in 1997, the Nikkei Environmental Technology
Award from Nihon Keizai Shinbun, Inc., in 2004, and thePrime Minister Award from Cabinet Office of Japan in
2004. His current research interests are TiO2 photocatalysis for environmental purifications, photo-functionalized
molecular magnets and organic photovoltaic devices.

Hiroshi Irie studied Inorganic Materials Scienceand received his B.E. and
M.E. degrees from Tokyo
Institute of Technology in1992 and 1994, respectively. From 1994 to 1997,
he served at Sumitomo
Metal Industries, Ltd., as a
research engineer. In 2000,
he received his Ph. D. degree from the University of Tokyo in the Department of Interdisciplinary Studies. He
was a postdoctoral fellow with the University of Tokyo
until the end of 2000 and a research staff member at
Kanagawa Academy of Science and Technology until
2001. He joined Research Center for Advanced Scienceand Technology at the University of Tokyo as a research
associate in 2001. Now, he belongs to Department ofApplied Chemistry at the same University. He has been
awarded the Promotion of Research in the 19th Electroceramics Research Conference of the Ceramic Societyof Japan. His current research interests are creations ofhigh-performance photocatalytic TiO2, novel photocatalytic materials, and TiO2 with new functions.

Akira Fujishima received
his B.E. degree in Electrochemistry from Yokohama National University in1966. He received his M.E.
from the University of Tokyo in 1968 and his Ph. D.
from the same University
in 1971. He became a lecturer in 1971 and an associate professor in 1973 at Kanagawa University. Again,
he joined the University of Tokyo as a lecturer in 1975.
He became an associate professor at the University ofTokyo from 1978 and was promoted to full professor
in 1986. In 2003, he was awarded professor emeritus
from the University of Tokyo. Presently, he is the Chairman of Kanagawa Academy of Science and Technology.
He served as the President of various scientific societies,
the Japanese Association of Photochemistry, the Electrochemical Society of Japan, and the Chemical Society ofJapan. He has received several awards for his research
excellence from various societies, such as the Electrochemical Society of Japan, the Chemical Society of Japan, and the Federation of Asian Chemical Societies. In
2004, he has been awarded the Japan Academy Prizeand the Japan Prize for Science. His current research interests include TiO2 photocatalysis and the electrochemistry of boron-doped diamond electrodes.

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JSAP International No.14 (July 2006)